Tartaric acid is a solid diprotic acid at room temperature found naturally in grapes.
Calculate the mass of tartaric acid (H2C4H4O6\text{H}_2\text{C}_4\text{H}_4\text{O}_6H2C4H4O6) needed to make 250 cm3250\text{ cm}^3250 cm3 of a standard solution with a concentration of 0.0600 mol/dm30.0600\text{ mol/dm}^30.0600 mol/dm3.
Relative formula mass (MrM_rMr): H2C4H4O6=150\text{H}_2\text{C}_4\text{H}_4\text{O}_6 = 150H2C4H4O6=150
A student carried out a titration and found that 25.0 cm325.0\text{ cm}^325.0 cm3 of a potassium hydroxide (KOH\text{KOH}KOH) solution was completely neutralised by 15.50 cm315.50\text{ cm}^315.50 cm3 of the 0.0600 mol/dm30.0600\text{ mol/dm}^30.0600 mol/dm3 tartaric acid solution.
The equation for the reaction is:
H2C4H4O6+2KOH→K2C4H4O6+2H2O \text{H}_2\text{C}_4\text{H}_4\text{O}_6 + 2\text{KOH} \rightarrow \text{K}_2\text{C}_4\text{H}_4\text{O}_6 + 2\text{H}_2\text{O} H2C4H4O6+2KOH→K2C4H4O6+2H2OCalculate the concentration of the potassium hydroxide solution in mol/dm3\text{mol/dm}^3mol/dm3.
40 exam-style questions on AQA GCSE Chemistry 4.2 Reactions of acids, covering 4.2.1 Reactions of acids with metals, 4.2.2 Neutralisation of acids and salt production, 4.2.3 Soluble salts, 4.2.4 The pH scale and neutralisation, 4.2.5 Titrations, and 4.2.6 Strong and weak acids (HT only). Each one has a worked solution and a mark scheme showing where the marks go.